Solubility Multiple Choice

Solubility Multiple Choice August 1998 13) In 0.20M Na 2 CrO 4, the ion concentrations are [Na + ] [CrO 2-4 ] A 0.40M 0.20M B 0.20M 0.20M C 0.20M 0.40M D 0.40M 0.80M 14) Which of the following compounds is the least soluble in water? A. H 2 S B. KNO 3 C. ZnSO 4 D. Ca(OH) 2 15) Which of the following 0.20M solutions will not form a precipitate when mixed with an equal volume of 0.20M Sr(OH) 2? A. CaS B. NH 4 Cl C. Na 2 SO 4 D. Ba(NO 3 ) 2 16) Consider the following equilibrium: SrF 2 (s) Sr 2 + (aq) + 2F - (aq) The equilibrium will shift left upon the addition of A. H 2 O (l) B. SrF 2 (s) C. SrCl 2 (s) D. NaNO 3 (s) 17) Two ions found in hard water are Ca 2+ and Mg 2+. Which of the following will precipitate only one of these ions? A. I - B. S 2- C. SO 4 2- D. CO 3 2-

18) At 25, the solubility of AgBr is A. 2.9 10-25 M B. 5.4 10-13 M C. 2.7 10-13 M D. 7.3 10-7 M 19) Which of the following saturated solutions has the greatest [CO 3 2- ]? A. SrCO 3 B. CaCO 3 C. BaCO 3 D. MgCO 3 January 1999 14. Which of the following units could be used to describe solubility? A. g/s B. g/l C. M/L D. mol/s 15. Consider the following anions: When 10.0mL of 0.20M Pb(NO3) 2 are added to each of the above, precipitates form in: A. I and II only. B. I and III only. C. II and III only. D. I, II and III. 16. When equal volumes of 0.20M CuSO4 and 0.20M Li 2 S are combined, the complete ionic equation is: A. Cu 2+ (aq) + S 2 (aq) CuS (s) B. CuSO 4 (aq) + Li 2 S (aq) CuS (s) + Li 2 SO 4 (aq) C. Cu 2+ (aq) +SO 4 2 (aq) + 2Li + (aq) + S 2 (aq) Li 2 SO 4 (aq) + CuS (s) D. Cu 2+ (aq) +SO 4 2 (aq) +2Li + (aq) +S 2 (aq) CuS (s) + 2Li + (aq) + SO 4 2 (aq)

17. The Ksp expression for a saturated solution of Ag2CO3 is A. Ksp = [Ag 2 + ][CO 3 2- ] B. Ksp = [Ag + ] 2 [CO3-2 ] C. Ksp = [2Αg + ][CO3-2 ] D. Ksp = [2Αg + ] 2 [CO3-2 ] 18. The solubility of FeF2 is 8.4 10 3 M. The Ksp value is A. 5.9 10 7 B. 2.4 10 6 C. 7.1 10 5 D. 8. 4 10 3 19. If the Trial Ion Product for AgBrO3 is calculated to be 1.0 10 7, then A. a precipitate forms because the Trial Ion Product > Ksp B. a precipitate forms because the Trial Ion Product < Ksp C. no precipitate forms because the Trial Ion Product > Ksp D. no precipitate forms because the Trial Ion Product < Ksp 20. The least soluble salt in water is A. CaS B. CaSO4 C. CaC2O4 D. Ca(NO3) 2 April 1999 14. Which of the following produces a molecular solution when dissolved in water? A. RbClO B. CH3OH C. NH4SCN D. NaCH3COO

15. Consider the solubility equilibrium: CaCO 3(s) Ca 2+ (aq) + CO 3 2- (aq) An additional piece of solid CaCO3 is added to the equilibrium above. The rate of dissolving and rate of crystallization have 16. At 25 C, which of the following compounds would dissolve to form a saturated solution with the greatest [Pb 2+ ]? A. PbI2 B. PbCl2 C. PbBr2 D. Pb(IO 3 ) 2 17. When equal volumes of 0.20M ZnSO4 and 0.20M Sr(OH)2 are combined, A. no precipitate forms. B. a precipitate of only SrSO4 forms. C. a precipitate of only Zn(OH)2 forms. D. precipitates of both SrSO4 and Zn(OH)2 form. 18. The solubility of SnS is 3.2 10 3 M. The value of Ksp is A. 1. 0 10 5 B. 3.2 10 3 C. 6.4 10 3 D. 5.7 10 2 19. Silver chloride, AgCl, would be least soluble in A. 1.0M HCl B. 1.0M NaNO3 C. 1.0M ZnCl2 D. 1.0M AgNO3

20. The solubility of SrF2 is A. 4.3 10 9 M B. 6.6 10 5 M C. 1.0 10 3 M D. 1.6 10 3 M June 1999 14. The ion concentrations in 2.00L of 0.32M K3PO4 are 15. Which of the following compounds is the least soluble in water? A. CaS B. Fe (OH) 3 C. KMnO4 D. NH4HC2O4 16. A solution contains two cations, each having a concentration of 0.20M. When an equal volume of 0.20M OH is added, these cations are removed from the solution by precipitation. These ions are: A. Ba 2+ and K + B. Sr 2+ and Na + C. Mg 2+ and Sr 2+ D. Mg 2+ and Ca 2+ 17. The solubility of Mn(IO 3 ) 2 is 4.8 10 3 M. What is the value of Ksp? A. 1.1 10 7 B. 4.4 10 7 C. 7.1 10 6 D. 1.1 10 1

18. The maximum [SO 4 2- ] that can exist in 1.0 10 3 M Ca(NO 3 ) 2 without a precipitate forming is: A. 7.1 10 5 M B. 1. 0 10 3 M C. 8. 4 10 3 M D. 7.1 10 2 M August 1999 14. Consider the following solutes: Which of the solutes above form only molecular aqueous solutions? A. I and II B. II and III C. II, III and IV D. I, II, III and IV 15. At a certain temperature, 7.0 10 4 mol MgSO4 is present in 100.0mL of solution. The concentration of the Mg 2+ in this solution is A. 7.0 10 5 M B. 7.0 10 4 M C. 7.0 10 3 M D. 7.0 10 6 M 16. When equal volumes of 0.20M SrBr2 and 0.20M AgNO3 are combined, A. no precipitate forms. B. a precipitate of only AgBr forms. C. a precipitate of only Sr(NO3)2 forms. D. precipitates of both AgBr and Sr(NO 3 ) 2 form.

17. Consider the following solubility equilibrium: PbCl2 (s) Pb 2+ (aq) + 2Cl - (aq) A student adds NaCl (s) to a saturated solution of PbCl2. When equilibrium is reestablished, how have the concentrations changed from the original equilibrium? A. [Pb 2+ ] and [Cl - ] both increased. B. [Pb 2+ ] and [Cl - ] both decreased. C. [Pb 2+ ] decreased and [Cl - ] increased. D. [Pb 2+ ] increased and [Cl - ] decreased. 18. Solid Ag2CrO4 is added to water to form a saturated solution. The Ksp value can be calculated by: A. Ksp = [CrO4 2- ] 2 B. Ksp = [CrO4 2- ] 3 C. Ksp = [CrO4 2- ] 3 2 D. Ksp = 4 [CrO4 2- ] 3 19. Consider the following solubility equilibrium: BaSO3 (s) Ba 2+ (aq) + SO3 2- (aq) Which of the following will result in an increase of [Ba 2+ ]? A. adding water B. adding BaS (s) C. adding BaSO3 (s) D. adding Na2SO3 (s) 20. When equal volumes of 0.20M Ca(NO 3 ) 2 and 0.20M Na2SO4 are combined, A. a precipitate forms because Trial Ion Product > Ksp B. a precipitate forms because Trial Ion Product < Ksp C. no precipitate forms because Trial Ion Product > Ksp D. no precipitate forms because Trial Ion Product < Ksp

21. Solid NaBrO3 is added to a 0.010M Ag + solution. What is the [BrO3 - ] when a precipitate first forms? A. 2.8 10 9 M B. 5.3 10 7 M C. 5.3 10 3 M D. 1. 0 10 2 M January 2000 14. Which of the following does not define solubility? A. the concentration of solute in a saturated solution B. the moles of solute dissolved in a given volume of solution C. the maximum mass of solute that can dissolve in a given volume of solution D. the minimum moles of solute needed to produce one litre of a saturated solution 15. The ion concentrations in 0.25 M Al 2 (SO 4 ) 3 are 16. Which of the following will not produce a precipitate when equal volumes of 0.20 M solutions are combined? A. KOH and CaCl2 B. Zn(NO 3 ) 2 and K 3 PO 4 C. Sr(OH) 2 and (NH 4 ) 2 S D. Na 2 SO 4 and Pb(NO 3 ) 2 17. What is observed when H 2 SO4 is added to a saturated solution of CaSO4? A. the ph increases B. the [Ca 2+ ]increases C. bubbles of H2 are given off D. additional CaSO4 precipitates

18. The solubility of CdS = 2.8 x 10-14. The value of Ksp is A. 7.8 x 10-28 B. 2.8 x 10-14 C. 5.6 x 10-14 D. 1.7 x 10-7 19. How many moles of solute are dissolved in 200.0 ml of a saturated solution of FeS? A. 1.2 x 10-19 B. 6.0 x 10-19 C. 1.5 x 10-10 D. 7.7 x 10-10 20. Consider the following 10.0 ml solutions: Equal moles of AgNO3 are added to each solution. It is observed that a precipitate forms in all but one solution. Which solution does not form a precipitate? A. Cl - B. Br - C. IO3 - D. BrO3-21. Which of the following could dissolve a precipitate of CaC 2 O 4 in a saturated solution of CaC 2 O 4? A. NaOH B. CaC 2 O 4 C. H 2 C 2 O 4 D. Ca(NO3)2

April 2000 14. Which of the following will dissolve in water to produce a molecular solution? A. CaCl2 B. NaOH C. CH 3 OH D. Sr(OH)2 15. In a solubility equilibrium, the A. rate of dissolving equals the rate of crystallization. B. neither dissolving nor crystallization are occurring. C. concentration of solute and solvent are always equal. D. mass of dissolved solute is greater than the mass of the solution. 16. Which of the following solutions would have [Fe +3 ] = 0.020 M? A. 0.40 L of 0.050 M Fe(NO 3 ) 3 B. 0.80 L of 0.020 M Fe 2 (SO 4 ) 3 C. 0.50 L of 0.040 M FeC 6 H 5 O 7 D. 0.50 L of 0.010 M Fe 2 (C 2 O 4 ) 3 17. Which of the following substances has the lowest solubility? A. BaS B. CuS C. FeS D. ZnS 18. The complete ionic equation for the reaction between MgS and Sr(OH)2 is A. MgS (aq) + Sr(OH) 2(aq) Mg(OH) 2(s) + SrS (s) B. MgS (aq) + Sr(OH) 2(aq) Mg(OH) 2(s) + SrS (aq) C. Mg +2 (aq) + S -2 (aq) + Sr +2 (aq) + 2OH - (aq) Mg +2 (aq) + 2OH - (aq) + SrS (s) D. Mg +2 (aq) + S -2 (aq) + Sr +2 (aq) + 2OH - (aq) Mg(OH) 2(s) + S -2 (aq) + Sr +2 (aq) 19. Consider the following equilibrium: Fe(OH) 2(s) Fe +2 (aq) + 2OH - (aq) Which of the following will cause the equilibrium to shift to the right? A. adding KOH B. adding Na 2 S C. adding Fe(OH) 2 D. adding Fe(NO3)2

20. Consider the following experiment: The unknown solution could contain A. 0.20 M OH - B. 0.20 M NO 3 - C. 0.20 M PO 4-3 D. 0.20 M SO 4-2 21. A compound has a solubility of 7.1 x 10-5 M at 25 C. The compound is A. CuS B. AgBr C. CaCO3 D. CaSO4 June 2000 14. A saturated solution of NaCl contains 36.5 g of solute in 0.100L of solution. The solubility of the compound is A. 0.062 M B. 1.60 M C. 3.65 M D. 6.24 M 15. Calculate the [Li + ] in 200.0 ml of 1.5 M Li 2 SO 4 A. 0.30 M B. 0.60 M C. 1.5 M D. 3.0 M

16. When equal volumes of 0.20 M RbCl and 0.20 M and M SrS are combined, A. no precipitate forms. B. a precipitate of Rb 2 S only forms. C. a precipitate of SrCl2 only forms. D. precipitates of both Rb 2 S and SrCl2 form. 17. A solution contains both Ag + and Mg 2+ ions. During selective precipitation, these ions are removed one at a time by adding A. I - followed by OH - B. OH - followed by S 2- C. SO4 2- followed by Cl - D. NO3 - followed by PO4 3-18. The Ksp expression for a saturated solution of Mg(OH)2 is 19. Consider the following saturated solutions: CuSO 4, BaSO 4, CaSO 4 The order of cation concentration, from highest to lowest, is A. [Ba 2+ ] > [Ca 2+ ] > [Cu 2+ ] B. [Ca 2+ ] > [Cu 2+ ] > [Ba 2+ ] C. [Cu 2+ ] > [Ca 2+ ] > [Ba 2+ ] D. [Cu 2+ ] > [Ba 2+ ] > [Ca 2+ ] 20. When 1.0 x10-3 moles of CuCl 2 (s) are added to 1.0 L of 1.0 x10-3 M IO 3 -, the A. Trial K sp > K sp and a precipitate forms. B. Trial K sp < K sp and a precipitate forms. C. Trial K sp > K sp and no precipitate forms. D. Trial K sp < K sp and no precipitate forms.

August 2000 14. Which of the following forms a molecular solution in water? A. SrSO4 B. Na 3 PO4 C. C 6 H 12 O 6 D. NH 4 CH 3 COO 15. Which of the following is necessary to form a saturated solution at equilibrium? A. excess solute B. an ionic solute C. solute of low solubility D. trial ion product is less than Ksp 16. The net ionic equation that describes a saturated solution of Ag 2 CrO4 is A. Ag 2 CrO 4 (s) Ag 2 CrO4 (aq) B. Ag 2 CrO 4 (s) 2Ag + (aq) + CrO4 2 (aq) C. Ag 2 CrO 4 (s) 2Ag + (aq) + Cr +6 (aq) + 4O -2 (aq) D. 2Ag + (aq) + CrO4 2 (aq) + 2H 2 O (l) 2AgOH (s) + H 2 CrO 4 (aq) 17. Which of the following compounds has the lowest solubility? A. SrS B. CaCl2 C. Rb 2 CO3 D. Zn(OH)2 18. Which of the following will form a precipitate when equal volumes of 0 2. M solutions are combined? A. HI and Na 2 CO3 B. SrS and NH 4 OH C. BaCl 2 and CuSO4 D. Mg(NO 3 ) 2 and KCl

19. The solute AgBr is least soluble in A. H 2 O B. 1.0 M FeBr 3 C. 1.0 M CaBr 2 D. 1.0 M AgNO 3 20. The magnesium and calcium ions in hard water can be removed by the addition of A. NaI B. NaNO3 C. Na 2 CO3 D. Na 2 SO4 21. The solubility of an AB2 type salt is 2.3 x 10 6 M. The salt is A. PbBr2 B. Fe(OH)2 C. Cu(IO3) 2 D. Mg(OH)2 22. Which of the following saturated solutions will have the lowest [Pb 2+ ]? A. PbI2 B. PbCl2 C. Pb(IO3)2 D. Pb(NO3) 2 January 2001 14. A saturated solution forms when a 0.10 mol of salt is added to 1.0L of water. The salt is A. Li2S B. CuBr2 C. Zn(OH)2 D(. (NH 4 )) 2 CO 3 15. Consider the following equilibrium: Ca(OH) 2 (s) Ca+2 (aq) + 2OH - (aq) Adding which of the following could cause the equilibrium [Ca +2+ ] to increase? A. H 2 O (l) B. HCl (aq)) C. KOH (s)) D. Ca((OH)) 2 ((s))

16. Consider the following solubility equilibrium: AgCl (s)) Ag + ( + (aq) + Cl (aq) Which of the following graphs represents the [Ag + ]+ after equilibrium has been established? 17. The concentrations of the cation and anion in 0.40 M (NH 4 ) 2 Cr 2 O 7 (aq) are 18. Which of the following will produce a solution with the highest [OH - ]? A. AgOH B. Sr(OH) 2 C. Fe(OH) 3 D. Mg(OH) 2 19. When equal volumes of 0.20 M ZnSO 4 and 0.20 M SrS are combined A. a precipitate does not form. B. a precipitate of only ZnS forms. C. a precipitate of only SrSO 4 forms. D. precipitates of both ZnS and SrSO 4 form.

20. What is the concentration of Pb 2+ in a saturated solution of Pb(IO 3 ) 2? A. 9.0 x 10-5 M B. 5.7 x 10-5 M C. 4.5 x 10-5 M D. 1.1 x 10-4 M April 2001 14. Which of the following dissolves in water to form a molecular solution? A. KCl B. Na 2 O C. NH 4 Br D. C 2 H 5 OH 15. A saturated solution is formed by adding 10.0g PbI 2 (s) to 10.0 ml of water in a beaker. Describe the situation which exists in the beaker. A. [Pb 2+ ] = [I - ] B. moles PbI 2 (s) = moles Pb +2 (aq) C. mass of PbI 2 (s) = mass of PbI 2 (aq) D. rate of crystallization = rate of dissociation 16. What is the concentration of barium ions in a 1.00 L solution containing 2.08 g of BaCl 2? A. 1.00 x 10-2 M B. 1.21 x 10-2 M C. 2.00 x 10-2 M D. 2.08 M 17. Which of the following salts has low solubility? A. MgS B. ZnCl 2 C. SrSO 4 D. AgNO 3

18. Consider the following solubility equilibrium: AgCl (s)) Ag + ( + (aq) + Cl (aq) Some NaCl (s) is added to the equilibrium. When equilibrium is reestablished, how have the ion concentrations changed from the original equilibrium? 19. A precipitate forms when a 0.20 M solution containing an unknown cation is added to SO 4 2-, but not when an equal volume is added to S 2-. The unknown cation is A. Na + B. Ca 2+ C. Pb 2+ D. Zn 2+ 20. The Ksp expression for a saturated solution of Ni 3 (PO 4 ) 2 is A. Ksp = [Ni +2 ] 3 [PO 4-3 ] 2 B. Ksp = [Ni +2 ] 2 [PO 4-3 ] 3 C. Ksp = [3Ni +2 ][2PO 4-3 ] D. Ksp = [3Ni +2 ] 3 [2PO 4-3 ] 2

June 2001 15. Consider the following equilibrium: BaSO 4 (s)) Ba +2 (aq) + SO 4 2 (aq) Adding which of the following will cause more solid BaSO4 to form? A. CaCl2 (s) B. K 2 CO3 (s) C. Na 2 SO4 (s) D. Mg(NO3)2 (s) 16. Which of the following could not be used to represent solubility? A. g/ml B. ml/l C. mol/l D. g/min 17. The following three beakers each contain different volumes of a saturated solution of PbI2 and different masses of solid PbI2 : What is the relationship for the [Pb 2+ ] in the solution in the three beakers? A. I = II = III B. I > II > III C. II > III > I D. III > II > I 18. The equation that describes the solubility equilibrium of Ag 2 CrO4 is A. Ag 2 CrO 4 (s) Ag 2 +2 (aq) + CrO 4-2 (aq) B. Ag 2 CrO 4 (s) 2Ag + (aq) + CrO 4-2 (aq) C. Ag 2 CrO 4 (s) 2Ag (s) + Cr (s) + 2O 2 (s) D. Ag 2 CrO 4 (s) 2Ag + (aq) + Cr +6 (aq) + 4O -2 (aq)

19. When 10.0 ml 0.20 M Zn(NO 3 ) 2 is added to a 10.0 ml sample of 0.20 M unknown solution, no precipitate forms. When the same volume of 0.20 M Ca(NO 3 ) 2 is added to a separate 10.0 ml sample of the unknown solution, a precipitate does form. The identity of the unknown solution could be A. NaCl B. Na 2 S C. Na 2 SO4 D. Na 2 CO3 20. The solubility of PbS is 1.8 x 10-14 M. The value of Ksp is A. 3.2 x 10-28 B. 1.8 x 10-14 C. 3.6 x 10-14 D. 1.3 x 10-7 August 2001 13. At 25 C, which of the following compounds has a low solubility when added to water? A. FeS B. CuCl2 C. ZnSO4 D. NH 4 CH 3 COO 14. Which of the following forms a molecular solution? A. KCl B. NaOH C. CH 3 OH D. NH 4 CH 3 COO

15. List the compounds AgI, KBr and MgCO3 in order of solubility from lowest to highest. A. AgI, MgCO 3, KBr B. KBr, AgI, MgCO3 C. KBr, MgCO 3, AgI D. MgCO 3, AgI, KBr 16. Consider the following Ksp expression: Ksp = [Cu +2 ][IO 3 - ] 2 Which of the following does this equilibrium expression represent? A. CuIO 3 (s) Cu + - (aq) + IO 3 (aq) B. CuIO 3 (s) Cu 2+ 2- (aq) + IO 3 (aq) C. CuIO 3 (s) Cu 2+ - (aq) + IO 3 (aq) D. Cu(IO 3 ) 2 (s) Cu 2+ - (aq) + 2IO 3 (aq) 17. The solubility of NiCO3 is 3.8 x 10-4 mol/l. The Ksp value is A. 1.4 x 10-7 B. 3.8 x 10-4 C. 7.6 x 10-4 D. 1.9 x 10-2 18. The [Ag + ] in a saturated solution of AgBrO3 is A. 2.8 x 10-9 M B. 2.6 x 10-5 M C. 5.3 x 10-5 M D. 7.3 x 10-3 M 19. When solutions of AgNO3 and NaCl are combined, the Trial Ksp for AgCl is 5.6 x 10-11. Predict what will be observed. A. a precipitate will form because Trial Ksp < Ksp B. a precipitate will form because Trial Ksp > Ksp C. a precipitate will not form because Trial Ksp < Ksp D. a precipitate will not form because Trial Ksp > Ksp

20. Calculate the maximum [CO3-2 ] that can exist in a solution without forming a precipitate when [Mg +2 ] = 0.20 M. A. 1.4 x 10-6 M B. 3.4 x 10-5 M C. 2.6 x 10-3 M D. 5.8 x 10-3 M January 2002 15) The equation that describes the solubility equilibrium of Ca 3 (PO 4 ) 2 is 6+ 3- A. Ca 3 (PO 4 ) 2(s) Ca 3 (aq) + 2PO 4 (aq) B. Ca 3 (PO 4 ) 2(s) 3Ca 2+ 3- (aq) + 2PO 4 (aq) C. Ca 3 (PO 4 ) 2(s) 2Ca 3+ 2- (aq) + 3PO 4 (aq) D. Ca 3 (PO 4 ) 2(s) (Ca 2+ ) 3(aq) + (PO 3-4 ) 2(aq) 16) In a saturated solution of Ag 2 C 2 O 4 the [Ag + ] = 2.2 10-4 M. What is the solubility of Ag 2 C 2 O 4 in this solution? A. 4.3 10-11 M B. 1.1 10-4 M C. 2.2 10-4 M D. 4.4 10-4 M 17) When equal volumes of 0.2M solutions are mixed, which of the following combinations forms a precipitate? A. CaS and Sr(OH) 2 B. H 2 SO 4 and MgCl 2 C. (NH 4 ) 2 SO 4 and K 2 CO 3 D. H 2 SO 3 and NaCH 3 COO 18) A solution contains 0.2 M Zn 2+ and 0.2M Sr 2+. An equal volume of a second solution was added, forming a precipitate with Sr 2+ but not with Zn 2+. What is present in the second solution? A. 0.2M Cl - B. 0.2M OH - C. 0.2M SO4 2- D. 0.2M PO 4 3-

19) The K sp expression for a saturated solution of Ba 3 (AsO 4 ) 2 is A. K sp = [Ba 2+ ][AsO 4 3- ] B. K sp = [Ba 2+ ] 3 [AsO 4 3- ] 2 C. K sp = [3Ba 2+ ][2AsO 4 3-] D. K sp = [3Ba 2+ ] 3 [2AsO 4 3- ] 2 20) The solubility of NiCo 3 is 4.4 10-2 g/l. Determine the K sp value of NiCO 3. A. 1.4 10-7 B. 3.7 10-4 C. 1.9 10-3 D. 2.1 10-1 21) Calculate the solubility of PbSO 4. A. 3.2 10-16 M B. 1.8 10-8 M C. 3.6 10-8 M D. 1.3 10-4 M 22) When a solution containing Ag + is mixed with a solution containing BrO 3 -, the trial ion product is determined to be 2.5 10-7. What would be observed? April 2002 A. A precipitate would form since trial ion product < K sp. B. A precipitate would form since trial ion product > K sp. C. A precipitate would not form since trial ion product < K sp. D. A precipitate would not form since trial ion product > K sp. 15) Which of the following will dissolve in water to form an ionic solution? A. O 2 B. CH 4 C. NH 4 Cl D. CH 3 OH 16) The solubility of SrCO 3 is 2.4 10-5 M. How many moles of dissolved solute are present in 100.0 ml of saturated SrCO 3 solution? A. 5.6 10-10 mol B. 2.4 10-6 mol C. 2.4 10-5 mol D. 2.4 10-4 mol

17) What are the ion concentrations in 0.30M CuCl2? [Cu 2+ ] [Cl - ] A. 0.10 M 0.20 M B. 0.20 M 0.10 M C. 0.30 M 0.30 M D. 0.30 M 0.60 M 18) What is the net ionic equation for the reaction that occurs when equal volumes of 0.20M Ba(NO 3 ) 2 and 0.20 M Na 2 SO 4 are mixed together? A. Ba 2+ (aq) + SO4 2- (aq) BaSo 4(s) B. Na +(aq) + NO 3 - (aq) NaNO 3(s) C. Ba(NO 3 ) 2(aq) + Na 2 SO 4 (aq) BaSO 4(s) + 2NaNO 3(aq) D. Ba 2+ (aq) + 2NO 3 - (aq) + 2Na + (aq) + SO 4 2- (aq) BaSO 4(s) + 2Na + (aq) + 2NO 3 - (aq) 19) Consider the following equilibrium: AgIO 3(s) Ag + (aq) + IO 3 - (aq) A few crystals of NaIO 3 are added to the above equilibrium. When equilibrium is re-established, how do the new ion concentrations compare with the original equilibrium concentrations? [Ag+] [IO3-] A. Decreased Decreased B. Decreased Increased C. Increased Decreased D. Increased Increased 20) The K sp expression for Zn(OH)2 is A. K sp = [Zn 2+ ][OH - ] 2 B. K sp = [Zn 2+ ] 2 [OH - ] C. K sp = [Zn 2+ ][2OH - ] D. K sp = [Zn 2+ ][2OH - ] 2

21) The solubility of CdCO 3 is 2.5 10-6 M. Calculate the K sp value for CdCO 3. June 2002 A. 6.3 10-12 B. 2.5 10-6 C. 5.0 10-6 D. 1.6 10-3 15) In every solubility equilibrium, the rate of dissolving is A. equal to zero. B. equal to the rate of crystallization C. less than the rate of crystallization D. greater than the rate of crystallization 16) A 3.0 L solution of BaCl 2 has a chloride ion concentration of 0.20 M. The barium ion concentration in this solution is A. 0.067 M B. 0.10 M C. 0.20 M D. 0.60 M 17) Which of the following has the lowest solubility? A. CaS B. CuS C. FeS D. MgS 18) What is the formula equation for the reaction that occurs when equal volumes of 0.20M K 3 PO 4 and 0.20M ZnCl 2 are mixed together? A. K + (aq) + Cl - (aq) KCl (s) B. 3Zn 2+ (aq) + 2PO 4 3- (aq) Zn 3 (PO 4 ) 2(s) C. 2K 3 PO 4(aq) + 3ZnCl 2(aq) Zn 3 (PO 4 ) 2(s) + 6KCl (aq) D. 2K 3 PO 4(aq) + 3ZnCl 2(aq) 3Zn 3 (PO 4 ) 2(aq) + 6KCl (s) 19) Which of the following could be added to a sample of hard water to remove both 0.2M Ca 2+ and 0.2M Mg 2+? A. 0.2 M S 2- B. 0.2 M Cl - C. 0.2 M OH - D. 0.2M So 4 2-

20) The K sp expression for a saturated solution of Ag 2 SO 3 is A. K sp = [2Ag + ][SO 3 2- ] B. K sp = [Ag + ] 2 [SO 3 2- ] C. K sp = [Ag 2 2+ ][SO 3 2- ] D. K sp = [2Ag + ] 2 [SO 3 2- ] 21) The solubility of CaF 2 is 3.3 10-4 M. Determine the K sp value of CaF 2. A. 3.6 10-11 B. 1.4 10-10 C. 1.1 10-7 D. 3.3 10-4 22) What is the maximum [Ag + ] that can exist in a solution of 0.010M NaIO 3? A. 3.2 10-10 M B. 3.2 10-8 M C. 3.2 10-6 M D. 1.8 10-4 M August 2002 15) Which of the following could be used to express solubility? A. mol B. M/s C. g/ml D. ml/min 16) When 100.0mL of a saturated solution of BaF 2 is heated and all the water is evaporated, 3.6 10-4 mol of solute remains. The solubility of BaF 2 is A. 1.9 10-10 M B. 1.3 10-5 M C. 3.6 10-4 M D. 3.6 10-3 M 17) A solution contains both 0.2M Mg 2+ (aq) and 0.2M Sr 2+ (aq). These ions can be removed separately through precipitation by adding equal volumes of 0.2M solutions of A. OH -, and then S 2- B. Cl -, and then OH - C. CO 3 2-, and then SO 3 2- D. SO 4 2-, and then PO 4 3-

18) Consider the following equilibrium: CaSO 4(s) Ca 2+ (aq) + SO 4 2- (aq) Which of the following would shift the above equilibrium to the left? A. adding CaSO 4(s) B. adding MgSO 4(s) C. removing some Ca 2+ (aq) D. removing some SO 4 2- (aq) 19) Calculate the solubility of CaC 2 O 4. A. 2.3 10-9 M B. 1.2 10-5 M C. 4.8 10-5 M D. 8.3 10-4 M 20) How many moles of dissolved solute are present in 100.0mL of a saturated SrCo3 solution? A. 5.6 10-11 mol B. 2.4 10-6 mol C. 2.4 10-5 mol D. 2.4 10-4 mol 21) What happens when equal volumes of 0.2M AgNO 3 and 0.2M NaCl are combined? A. A precipitate forms because the trial ion product > K sp B. A precipitate forms because the trial ion product < K sp C. No precipitate forms because the trial ion product > K sp D. No precipitate forms because the trial ion product < K sp 22) Determine the maximum [Na 2 CO 3 ] that can exist in 1.0L of 0.0010M Ba(NO 3 ) 2 without forming a precipitate. A. 2.6 10-12 M B. 2.6 10-9 M C. 2.6 10-6 M D. 5.1 10-5 M January 2003 15) Solid Ba(OH) 2 is added to water to prepare a saturated solution. Which of the following is true for this equilibrium system? A. [anion] = [cation] B. trial K sp is less than K sp C. blue litmus paper would turn red D. the rate of dissolving = the rate of crystallization

16) A saturated solution of PbI2 was subjected to a stress and the following graph was obtained. Which stress was applied at time t 1? A. the addition of PbI 2 B. a temperature change C. an increase in volume D. the evaporation of water 17) Which of the following would be true when equal volumes of 0.2M NaBr and 0.2M AgNO 3 are combined? A. No precipitate forms. B. A precipitate of AgBr forms. C. A precipitate of NaNO 3 forms. D. Precipitates of both NaNO 3 and AgBr form. 18) Using the solubility table, determine which of the following ions could not be used to separate S 2- from SO 4 2- by precipitation? A. Be 2+ B. Ca 2+ C. Ba 2+ D. Sr 2+ 19) Which of the following is true when solid Na 2 S is added to a saturated solution of CuS and equilibrium is reestablished? A. [S 2- ] increases. B. [Cu 2+ ] increases. C. [S 2- ] does not change. D. [Cu 2+ ] does not change.

20) Which of the following describes the relationship between the solubility product constant (K sp ) and the solubility (s) of PbI 2? A. Ksp = S2 B. Ksp = 4S3 21) Which of the following saturated solutions will have the lowest [S 2- ]? A. BaS B. CaS C. CuS D. ZnS 22) What is the solubility of SrF 2? April 2003 A. 3.2 10-25 M B. 1.8 10-17 M C. 4.3 10-9 M D. 1.0 10-3 M 15) Which of the following is a suitable term for representing solubiltity? A. grams B. moles C. molarity D. milliliters per second 16) A saturated solution is prepared by dissolving a salt in water. Which of the following graphs cold represent the ion concentrations as the temperature is changed?

17) What is the concentration of OH - ions in 250mL of 0.20 M Sr(OH) 2? A. 0.050 M B. 0.10 M C. 0.20 M D. 0.40 M 18) What happens when 10.0mL of 0.2 M KOH is added to 10.0mL of 0.2M CuSO 4? A. No precipitate forms. B. A precipitate of K 2 SO 4 forms C. A precipitate of Cu(OH) 2 forms. D. Precipitates of K 2 SO 4 and Cu(OH) 2 form. 19) Solid NaCl is added to a saturated AgCl solution. How have the [Ag + ] and [Cl - ] changed when equilibrium has been reestablished? [Ag+] [Cl-] A. increased increase B. decreased increased C. increased decreased D. decreased decreased 20) Which of the following expressions represents [Fe 2+ ] in a saturated Fe(OH) 3 solution? 21) What is the value of K sp for Zn(OH) 2 if the solubility of Zn(OH) 2 is equal to 4.2 10-6 M? A. 1.0 10-2 B. 4.0 10-3 C. 1.8 10-11 D. 3.0 10-16

22) What is the maximum number of moles of Cl - that can exist in 500.0mL of 2.0M AgNO 3? A. 4.5 10-11 B. 9.0 10-11 C. 1.8 10-10 D. 1.8 10-9 June 2003 15) What is the concentration of the ions in 3.0 L of 0.50 M Al 2 (SO 4 ) 3? [Al 3+ ] [SO 2-4 ] A 0.33 M 0.50 M B 1.0 M 1.5 M C 1.5 M 1.5 M D 3.0 M 4.5 M 16) Consider the following equilibrium: MgCO 3(s) Mg2 + (aq) + CO32 - (aq) Adding which of the following would cause the solid to dissolve? A. HCl B. K 2 CO 3 C. MgCO 3 D. Mg(NO 3 ) 2 17) Which of the following compounds could be used to prepare a solution with a [S 2- ] greater than 0.1 M? A. ZnS B. PbS C. Ag 2 S D. Rb 2 S 18) Which of the following will not form a precipitate when mixed with an equal volume of 0.2 M AgNO 3? A. 0.2 M NaBr B. 0.2 M NaIO 3 C. 0.2 M NaNO 3 D. 0.2 M NaBrO 3

19) A solution is prepared containing both 0.2 M OH - and 0.2 M PO 4 3- ions. An equal volume of a second solution is added in order to precipitate only one of these two anions. The second solution must contain which of the following? A. 0.2 M Cs + B. 0.2 M Zn 2+ C. 0.2 M Pb 2+ D. 0.2 M Sr 2+ 20) Consider the following equilibrium: CaS (s) Ca 2+ (aq) + S 2- (aq) When Ca(NO 3 ) 2(aq) is added to this solution, the equilibrium shifts to the A. left and [S 2- ] increases. B. left and [S 2- ] decreases. C. right and [S 2- ] increases. D. right and [S 2- ] decreases. 21) How many moles of Pb 2+ are there in 500.0mL of a saturated solution of PbSO 4? A. 3.2 10-16 B. 9.0 10-9 C. 6.7 10-5 D. 1.3 10-4 22) Which of the following compounds is least soluble in water? A. CuI B. BeS C. CsOH D. AgBrO 3 August 2003 15) Which of the following will dissolve to form a molecular solution? A. H 2 SO 4 B. AgNO 3 C. Ca(OH) 2 D. C 6 H 12 O 6

16) Consider the following equilibrium: energy + AgCl (s) Ag + (aq) + Cl - (aq) Addition of which of the following will increase the solubility of AgCl? A. heat B. HCl C. AgNO 3 D. a catalyst 17) What is the [Cl - ] when 15.0g of NaCl is dissolved in enough water to make 100.0mL of solution? A. 0.150 M B. 0.390 M C. 2.56 M D. 3.90 M 18) An equal number of moles of Na 2 CO 3 is added to four different 10.0mL samples. Sample 1 Sample 2 Sample 3 Sample 4 0.50 M Ba 2+ (aq) 0.50 M Ca 2+ (aq) 0.50 M Mg 2+ (aq) 0.50 M Sr 2+ (aq) A precipitate forms in only one of the samples. Identify the cation which is present in the precipitate. A. Ba 2+ B. Ca2 + C. Mg 2+ D. Sr 2+ 19) What is the net ionic equation of the reaction between BaS (aq) and Sr(OH) 2(aq)? A. Sr 2+ (aq) + S 2- (aq) SrS (s) B. Ba 2+ (aq) + 2OH - (aq) Ba(OH) 2(s) C. Ba 2+ (aq) + S 2- (aq) + Sr 2+ (aq) + 2OH - (aq) Ba(OH) 2(s) + SrS (s) D. Ba 2+ (aq) + S 2- (aq) + Sr 2+ (aq) + 2OH - (aq) Ba(OH) 2(s) + Sr 2+ (aq) +S 2- (aq) 20) In which of the following would PbCl2(s) be least soluble? A. 1 M HCl B. 1 M BaCl 2 C. 1 M K 2 SO 4 D. 1 M Pb(No 3 ) 2

21) The solubility of ZnCO 3 is 6.4 10-9 M. What is the value of K sp for ZnCO 3? A. 4.1 10-17 B. 6.4 10-9 C. 1.3 10-8 D. 8.0 10-5 22) When equal volumes of 0.20 M NaOH and 0.20 M CaS are mixed together, Solutions A. a precipitate forms and the Trial K sp would be less than K sp. B. no precipitate forms and the Trial K sp would be less than K sp. C. a precipitate forms and the Trial K sp would be greater than K sp. D. no precipitate forms and the Trial K sp would be greater than K sp. August 1998 13 A 14 D 15 B 16 C 17 C 18 D 19 D January 1999 April 1999 June 1999 August 1999 14 B 14 B 14 D 14 B 15 D 15 A 15 B 15 C 16 D 16 B 16 D 16 B 17 B 17 D 17 B 17 C 18 B 18 A 18 D 18 D 19 D 19 C 19 B 20 C 20 C 20 A 21 C January 2000 April 2000 June 2000 August 2000 14 B 14 C 14 D 14 C 15 B 15 A 15 D 15 A 16 C 16 D 16 A 16 B 17 D 17 B 17 A 17 D 18 A 18 D 18 B 18 C 19 C 19 B 19 C 19 B 20 D 20 A 20 D 20 C 21 A 21 C 21 B 22 C

January 2001 April 2001 June 2001 August 2001 14 C 14 D 15 C 13 A 15 B 15 D 16 D 14 C 16 B 16 A 17 A 15 A 17 C 17 C 18 B 16 D 18 B 18 A 19 C 17 A 19 D 19 B 20 A 18 D 20 C 20 A 19 C 20 B January 2002 April 2002 June 2002 August 2002 15 B 15 C 15 B 15 C 16 B 16 B 16 B 16 D 17 A 17 D 17 B 17 D 18 C 18 A 18 C 18 B 19 B 19 B 19 C 19 C 20 A 20 A 20 B 20 B 21 D 21 A 21 B 21 A 22 C 22 C 22 C 22 C January 2003 April 2003 June 2003 August 2003 15 D 15 C 15 B 15 D 16 B 16 D 16 A 16 A 17 B 17 D 17 D 17 C 18 A 18 C 18 C 18 D 19 A 19 B 19 D 19 B 20 B 20 B 20 B 20 B 21 C 21 D 21 C 21 A 22 D 22 A 22 A 22 C